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| Names | |
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| IUPAC name
Caesium chloride
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| Other names
Cesium chloride
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.028.728 |
| EC Number |
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PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| CsCl | |
| Molar mass | 168.36 g/mol |
| Appearance | white solid hygroscopic |
| Density | 3.988 g/cm3[1] |
| Melting point | 646 °C (1,195 °F; 919 K)[1] |
| Boiling point | 1,297 °C (2,367 °F; 1,570 K)[1] |
| 1910 g/L (25 °C)[1] | |
| Solubility | soluble in ethanol[1] |
| Band gap | 8.35 eV (80 K)[2] |
| -56.7·10−6 cm3/mol[3] | |
Refractive index (nD)
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1.712 (0.3 μm) 1.640 (0.59 μm) 1.631 (0.75 μm) 1.626 (1 μm) 1.616 (5 μm) 1.563 (20 μm)[4] |
| Structure | |
| CsCl, cP2 | |
| Pm3m, No. 221[5] | |
a = 0.4119 nm
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Lattice volume (V)
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0.0699 nm3 |
Formula units (Z)
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1 |
| Cubic (Cs+) Cubic (Cl−) | |
| Hazards | |
| GHS labelling: | |
 
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| Warning | |
| H302, H341, H361, H373 | |
| P201, P202, P260, P264, P270, P281, P301+P312, P308+P313, P314, P330, P405, P501 | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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2600 mg/kg (oral, rat)[6] |
| Related compounds | |
Other anions
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Caesium fluoride Caesium bromide Caesium iodide Caesium astatide |
Other cations
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Lithium chloride Sodium chloride Potassium chloride Rubidium chloride Francium chloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Caesium chloride or cesium chloride is the inorganic compound with the formula CsCl. This colorless salt is an important source of caesium ions in a variety of niche applications. Its crystal structure forms a major structural type where each caesium ion is coordinated by 8 chloride ions. Caesium chloride dissolves in water. CsCl changes to NaCl structure on heating. Caesium chloride occurs naturally as impurities in carnallite (up to 0.002%), sylvite and kainite. Less than 20 tonnes of CsCl is produced annually worldwide, mostly from a caesium-bearing mineral pollucite.[7]
Caesium chloride is widely used in isopycnic centrifugation for separating various types of DNA. It is a reagent in analytical chemistry, where it is used to identify ions by the color and morphology of the precipitate. When enriched in radioisotopes, such as 137CsCl or 131CsCl, caesium chloride is used in nuclear medicine applications such as treatment of cancer and diagnosis of myocardial infarction. Another form of cancer treatment was studied using conventional non-radioactive CsCl. Whereas conventional caesium chloride has a rather low toxicity to humans and animals, the radioactive form easily contaminates the environment due to the high solubility of CsCl in water. Spread of 137CsCl powder from a 93-gram container in 1987 in Goiânia, Brazil, resulted in one of the worst-ever radiation spill accidents killing four and directly affecting 249 people.
- ^ a b c d e Haynes, p. 4.57
- ^ Lushchik, A; Feldbach, E; Frorip, A; Ibragimov, K; Kuusmann, I; Lushchik, C (1994). "Relaxation of excitons in wide-gap CsCl crystals". Journal of Physics: Condensed Matter. 6 (12): 2357–2366. Bibcode:1994JPCM....6.2357L. doi:10.1088/0953-8984/6/12/009. S2CID 250824677.
- ^ Haynes, p. 4.132
- ^ Haynes, p. 10.240
- ^ Watanabe, M.; Tokonami, M.; Morimoto, N. (1977). "The transition mechanism between the CsCl-type and NaCl-type structures in CsCl". Acta Crystallographica Section A. 33 (2): 294. Bibcode:1977AcCrA..33..294W. doi:10.1107/S0567739477000722.
- ^ Cesium chloride. nlm.nih.gov
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.